Propane is C3H8
1 mole of propane has 3 carbon atoms and 8 hydrogen atoms.
1 mole of any substance has the Avogadro number 6.022 ×1023 particles/mol
Given mass = 20 grams
Molar mass is the sum of the atomic masses of all atoms present in the molecule:
So for propane:
Each Carbon atom has an atomic mass = 12 g / mol
Each Hydrogen atom has a atomic mass = 1 g / mol
So the molar mass of propane is (3 × 12) + (8× 1) = 44 g / mol
The percentage of Carbon in 1 mole of propane = (3 × 12) ×100 / 44 = 81.8%
Then the mass of carbon in 20 grams of propane = (81.8 × 20) / 100 = 16.36 g
Now 16.36 grams of Carbon corresponds to how many moles of Carbon
Number of moles = Available mass / Molar mass
Number of moles of carbon = 16.36 / 12 = 1.3633 moles
The number of atoms in any substance is defined as number of moles of that substance × Avogadro’s constant
So the number of carbon atoms in 20 grams of propane = 1.3633 mol ×6.022 × 1023 atoms / mol = 8.207 × 1023 atoms
Hence the number of carbon atoms in 20 grams of propane is 8.207 × 1023
Exercise 3.5 Calculate the number of carbon atoms in 20.0 g of propane, C3H8. 3(12.01)
A sample of propane, C3H8, contains 15.4 moles of carbon atoms. How many total moles of atoms does the sample contain? A sample of propane, C3Hs, contains 15.4 moles of carbon atoms. How many total moles of atoms does the sample contain? Express the total number of moles of carbon and hydrogen numerically. View Available Hint(s) moles Submit Previous Answers
Propane (C3H8) burns in oxygen to produce carbon dioxide and water via the following reaction: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calculate the mass of CO2 that can be produced if the reaction of 49.9 g of propane and sufficient oxygen has a 60.0 % yield.
27) When propane (C3H8) reacts with oxygen, carbon dioxide and water are produced. The balanced equation for this reaction is: C3H8 (g) + 5O2 (g) ---> 3CO2 (g) + 4H2O (g) Suppose 17.8 moles of oxygen react. The reaction consumes ___ moles of propane (C3H8). The reaction produces ___ moles of carbon dioxide and ___ moles of water. How many grams of water are produced in the complete reaction of 27.2 grams of propane (C3H8)? ___ grams
Calculate the amount of carbon dioxide produced when burning 10.0 g of propane with 5 g of oxygen in the following reaction. C3H8 + 5 O2 -------> 3 CO2 + 4 H2O
A 75.0 L steel tank at 20.0 degrees C contains propane gas, C3H8, at a pressure of 1.39 atm. Assuming ideal behavior, how many moles of C atoms are in the tank?
Question 3 Propane (C3H8) undergoes combustion according to the following thermochemical equation: C3H8(g) + 5 O2(g) -- 3 CO2(g) + 4H2O(g) Arxn = -2043.0 kJ Substance Heat of Formation (kJ/mol) CO2(g) -393.5 H2O(g) -241.8 O2(g) 0 C3H8(g) ? Calculate the standard enthalpy of formation of propane C3H8 a. -104.7 kJ/mol ob. +1407.7 kJ/mol C. -1407.7 kJ/mol O d. +104.7 kJ/mol o e. -4190.7 kJ/mol
A sample of C3H8 has 1.68×1024 H atoms. How many carbon atoms does the sample contain? number of carbon atoms: C atoms What is the total mass of the sample? mass: g C3H8
The combustion of propane can be represented by the following equation: __ C3H8 (g) + __O2(g) → __CO2(g) + __H2O(g) Balance the equation and answer the next three questions. If 257. g of C3H8 and 951. g O2 react, which reactant is used up first? (enter propane or oxygen) What is the mass of carbon dioxide produced? (Give your answer to 3 sig figs.) What is the mass of water produced?(Give your answer to 3 sig figs.) grams
A sample of C3H8 has 1.60×1024 H atoms. How many carbon atoms does the sample contain? number of carbon atoms: ?×10 ? C atoms What is the total mass of the sample? mass: ? ×10 ? g C3H8
Propane (C3H8)burns according to the following balanced equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calculate ΔH∘rxnΔ for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/molkJ/mol.) Express the enthalpy in kilojoules to four significant figures.